To solve both of these questions, we need to use the equilibrium expression and the given values to set up an equation. Let's start with the first question:
1. For the reaction CO(g) + Cl2(g) â COCl2(g), the equilibrium constant expression Kc is given as 2.50 (in M^-1).
To calculate the equilibrium molar concentration of CO, let's assume the equilibrium molar concentration of CO is x M. Since the initial molar concentration of CO is 1.40 mol and the change at equilibrium will be -x (as CO is being consumed in the forward reaction), the equilibrium molar concentration of CO will be (1.40 - x) M.
The equilibrium molar concentration of Cl2 is 3.20 mol, and the equilibrium molar concentration of COCl2 will also be (1.40 - x) M (as one mole of COCl2 is produced per mole of CO consumed in the forward reaction).
Using the equilibrium constant expression, we can set up the equation:
Kc = [COCl2] / ([CO][Cl2])
Substituting the equilibrium molar concentrations, we have:
2.50 = (1.40 - x) / ((1.40 - x)(3.20))
Simplifying the equation:
2.50 = 1 / 3.20
Now, solve for x to find the equilibrium molar concentration of CO. Multiply both sides by (1.40 - x)(3.20):
2.50(1.40 - x)(3.20) = 1
7.00 - 2.50x = 1
2.50x = 7.00 - 1
2.50x = 6.00
x = 6.00 / 2.50
x = 2.40 M
So, the equilibrium molar concentration of CO is 2.40 M.
Now let's move on to the second question:
2. For the reaction CO(g) + Cl2(g) â COCl2(g), we need to calculate Kp (in atm^-1) using the given pressure values.
Let's assume the equilibrium molar pressure of CO is x atm. Since the initial molar pressure of CO is 0.74 atm and the change at equilibrium will be -x, the equilibrium molar pressure of CO will be (0.74 - x) atm.
The equilibrium molar pressure of Cl2 is 0.92 atm, and the equilibrium molar pressure of COCl2 will also be (0.74 - x) atm.
Using the equilibrium constant expression in terms of partial pressures, we have:
Kp = (PCOCl2) / (PCO)(PCl2)
Substituting the equilibrium molar pressures, we have:
Kp = (0.74 - x) / ((0.74 - x)(0.92))
Simplifying the equation:
Kp = 1 / 0.92
Now, solve for x to find the equilibrium molar pressure of CO. Multiply both sides by (0.74 - x)(0.92):
Kp(0.74 - x)(0.92) = 1
(0.74 - x) / (0.74 - x) = 1 / Kp(0.92)
0.74 - x = 1 / Kp(0.92)
x = 0.74 - 1 / Kp(0.92)
x = 0.74 - 1.36
x = -0.62 atm (which is not possible)
It seems there may be an error in the given values or calculations for the second question. Please double-check the values and calculations.